(a)
To calculate: The pH of a 1L solution containing 10mL of 5M NaOH.
Concept introduction: The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution. The pH of a neutral aqueous solution is 7, therefore, if it exceeds 7, then it is a base and if it is below 7, then it is an acid.
(b)
To calculate: The pH of 10mL of 100mM glycine and 20mL of 5M HCl.
Concept introduction: The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution. The pH of a neutral aqueous solution is 7, therefore, if it exceeds 7, then it is a base and if it below 7, then it is an acid.
(c)
To calculate: The pH of 10mL of 2M acetic acid and 5g of sodium acetate.
Concept introduction: The pH of a solution is denoted as the negative logarithm of the hydrogen ion concentration of that solution. The pH in a solution decreases as H+ ion concentration increases in the solution. The pH of a neutral aqueous solution is 7, therefore, if it exceeds 7, then it is a base and if it below 7, then it is an acid.
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